posted by Sara .
The half-life for the second-order reaction of a substance A is 58.2 s when A0 = 0.63 mol L-1 Calculate the time needed for the concentration of A to decrease to the following values.
(a) one-third of its original value
(b) one-sixth of its original value
(c) one-seventh of its original value
What's wrong with substituting values into the second order equation and solving for time.
Could it be you don't know how to handle 1/3, 1/6, 1/7 th values?
If Ao = 0.63 then 1/3 that = ? for a; 1/6 that for b and 1/7 that for c.
I don't understand how to figure out K.
I used the information in the problem given to solve for k, and then plug that k in to solve for t, but it's not the correct answer.
t1/2 = [1/k(Ao)]
I understand, but what is K or how can I determine K?
The problem GIVES you the half life. Use that and the equation I provided above to determine k.